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Phase Transitions

Phase Transitions

Whether solid, liquid, or gas, a substance's state depends on the order and arrangement of its particles (atoms, molecules, or ions). Particles in the solid pack closely together, generally in a pattern. The particles vibrate about their fixed positions but do not move or squeeze past their neighbors. In liquids, although the particles are closely spaced, they are randomly arranged. The position of the particles are not fixed—that is, they are free to move past their neighbors to...

Phase Transitions: Melting and Freezing

Phase Transitions: Melting and Freezing

Heating a crystalline solid increases the average energy of its atoms, molecules, or ions, and the solid gets hotter. At some point, the added energy becomes large enough to partially overcome the forces holding the molecules or ions of the solid in their fixed positions, and the solid begins the process of transitioning to the liquid state or melting. At this point, the temperature of the solid stops rising, despite the continual input of heat, and it remains constant until all of the solid is...

Phase Transitions: Sublimation and Deposition

Phase Transitions: Sublimation and Deposition

Some solids can transition directly into the gaseous state, bypassing the liquid state, via a process known as sublimation. At room temperature and standard pressure, a piece of dry ice (solid CO2) sublimes, appearing to gradually disappear without ever forming any liquid. Snow and ice sublimate at temperatures below the melting point of water, a slow process that may be accelerated by winds and the reduced atmospheric pressures at high altitudes. When solid iodine is warmed, the solid sublimes...

Phase Diagram

Phase Diagram

The phase of a given substance depends on the pressure and temperature. Thus, plots of pressure versus temperature showing the phase in each region provide considerable insights into the thermal properties of substances. Such plots are known as phase diagrams. For instance, in the phase diagram for water (Figure 1), the solid curve boundaries between the phases indicate phase transitions (i.e., temperatures and pressures at which the phases coexist).

Phase Transitions: Vaporization and Condensation

Phase Transitions: Vaporization and Condensation

The physical form of a substance changes on changing its temperature. For example, raising the temperature of a liquid causes the liquid to vaporize (convert into vapor). The process is called vaporization—a surface phenomenon. Vaporization occurs when the thermal motion of the molecules overcome the intermolecular forces, and the molecules (at the surface) escape into the gaseous state. When a liquid vaporizes in a closed container, gas molecules cannot escape. As these gas phase molecules...

Entropy Change in Reversible Processes

Entropy Change in Reversible Processes

In the Carnot engine, which achieves the maximum efficiency between two reservoirs of fixed temperatures, the total change in entropy is zero. The observation can be generalized by considering any reversible cyclic process consisting of many Carnot cycles. Thus, it can be stated that the total entropy change of any ideal reversible cycle is zero.
The statement can be further generalized to prove that entropy is a state function. Take a cyclic process between any two points on a p-V diagram.

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Related Experiment Video

Updated: Dec 28, 2025

Orientational Transition in a Liquid Crystal Triggered by the Thermodynamic Growth of Interfacial Wetting Sheets

Orientational Transition in a Liquid Crystal Triggered by the Thermodynamic Growth of Interfacial Wetting Sheets

Published on: May 15, 2017

Electronic Griffiths Phase in Disordered Mott-Transition Systems.

Riku Yamamoto¹, Tetsuya Furukawa¹, Kazuya Miyagawa²

¹Department of Applied Physics, Tokyo University of Science, Tokyo 125-8585, Japan.

Physical Review Letters

|February 15, 2020

Summary

This summary is machine-generated.

Correlated electrons in solids exhibit soft-matter-like behavior, such as slow dynamics and self-organization, only when on the metal-insulator boundary and under quenched disorder. This phenomenon is explained by the electronic Griffiths phase.

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Methods of Ex Situ and In Situ Investigations of Structural Transformations: The Case of Crystallization of Metallic Glasses

Methods of Ex Situ and In Situ Investigations of Structural Transformations: The Case of Crystallization of Metallic Glasses

Published on: June 7, 2018

Area of Science:

Condensed Matter Physics
Soft Matter Physics
Materials Science

Background:

Solid-state and soft-matter physics have historically developed in isolation.
Correlated electron systems, particularly Mott-transition materials, exhibit behaviors analogous to soft matter, including self-organization and slow dynamics.

Purpose of the Study:

To investigate the conditions under which correlated electrons in solid matter display soft-matter-like characteristics.
To identify the key factors driving slow electron dynamics and self-organization in organic Mott-transition systems.

Main Methods:

Focused on an organic Mott-transition system.
Analyzed electron dynamics under varying conditions, specifically examining the metal-insulator boundary and the presence of quenched disorder.

Main Results:

Demonstrated that slow electron fluctuation occurs only when the system is simultaneously at the metal-insulator boundary and subjected to quenched disorder.
Identified this state of slow dynamics as the (electronic) Griffiths phase.

Conclusions:

The (electronic) Griffiths phase provides a framework for understanding slow electron dynamics in solids.
This finding offers a potential bridge connecting concepts between solid-state and soft-matter physics.